Question

1. how many moles of fe will be produced if 22.897 grams of co₂ are produced?

2 fe₂o₃ + 3 c → 4 fe + 3 co₂

Explanation:

Step1: Calculate moles of \(CO_2\)

The molar mass of \(CO_2\) is \(M = 12+2\times16=44\space g/mol\).
Using the formula \(n=\frac{m}{M}\), where \(m = 22.897\space g\) and \(M = 44\space g/mol\), we have \(n_{CO_2}=\frac{22.897}{44}\space mol\).

Step2: Use mole ratio from the balanced equation

From the balanced equation \(2Fe_2O_3 + 3C
ightarrow4Fe + 3CO_2\), the mole ratio of \(Fe\) to \(CO_2\) is \(n_{Fe}:n_{CO_2}=4:3\).
So \(n_{Fe}=\frac{4}{3}n_{CO_2}\).
Substitute \(n_{CO_2}=\frac{22.897}{44}\) into the above formula:
\(n_{Fe}=\frac{4}{3}\times\frac{22.897}{44}\)

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Answer:

\(0.694\space mol\)